At 90 °C the vapour pressure of toluene (methylbenzene) is 53 kPa and that of o-xylene (1,2-dimethylbenzene) is 20 kPa. (a) What is the molar fraction of toluene in the liquid mixture when the total vapor pressure is 0.50 atm at 90 °C? In liquid, xtoluene =........... At 90 °C the vapour pressure of toluene (methylbenzene) is 53 kPa and that of o-xylene (1,2-dimethylbenzene) is 20 kPa. (b) What is the molar fraction of toluene in the gas phase when the total vapor pressure is 0.50 atm at 90 °C? In gas, xtoluene = __________

At 90 °C the vapour pressure of toluene (methylbenzene) is 53 kPa and that of o-xylene (1,2-dimethylbenzene) is 20 kPa. (a) What is the molar fraction of toluene in the liquid mixture when the total vapor pressure is 0.50 atm at 90 °C? In liquid, xtoluene =........... At 90 °C the vapour pressure of toluene (methylbenzene) is 53 kPa and that of o-xylene (1,2-dimethylbenzene) is 20 kPa. (b) What is the molar fraction of toluene in the gas phase when the total vapor pressure is 0.50 atm at 90 °C? In gas, xtoluene = __________

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter17: Equilibrium

Section: Chapter Questions

Problem 13ALQ

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3. Assume that toluene and hexane form an ideal solution. At 365 K pure toluene has a vapour pressure of 0.582 bar and pure hexane has a vapour pressure of 1.99 bar. Consider a solution with mole fraction of hexane = 0.250. (a) Calculate the partial pressures of toluene and hexane, and the total pressure above the solution. (b) Some of the vapour is removed and allowed to condense in a second container. Calculate the partial pressures of hexane and toluene and the total pressure above this solution.
(b) At 80 °C, ethylene dibromide and propylene dibromide mixture forms an ideal solution. Given that the pure vapour pressures of ethylene dibromide and propylene dibromide are 22.9 and 16.9 kPa, respectively. Using the plots of partial vapour pressures of ethylene dibromide and propylene dibromide, and total vapour pressure of the mixture against the mole fraction of ethylene dibromide, determine (i) the composition of the vapour in equilibrium with a solution containing 0.75 mole fraction of ethylene dibromide. (ii) the composition of the liquid phase in equilibrium with ethylene dibromide- propylene dibromide containing 0.5 mole fraction each.
1,1-Dichloroethane (CH3CHCl2) has a vapour pressure of 228 torr at 25 °C; at the same temperature, 1,1-dichlorotetrafluoroethane (CF3CCl2F) has a vapour pressure of 79 torr. What mass of 1,1-dichloroethane must be mixed with 240.0 g of 1,1-dichlorotetrafluoroethane to give a solution with vapour pressure 157 torr at 25 °C? Assume ideal behaviour. (1 atm = 760 torr).
An open vessel containing (a) water, (b) benzene, (c) mercury stands in a laboratory measuring 5.0 m x 4.3 m x 2.2 m at 25 °c. The vapour pressures of each substance are (a) 2.3 kPa, (b) 10 kPa, (c) 0.30 Pa, respectively. What massof each substance will be found in the air if there is no ventilation?
8. Two l-litrc flask A and B are connected to each other by a valve which is closed. Flask A has benzene in equilibrium with its vapours at 30°C. The flask B, is evacualed, and the valve is opened. Which of the following is true. If temperature is kept constant. (a) Some of the benzene molecules would move to flask B fiom flask A. (b) Vapour pressurec will be halfthe initial valuc. (c) The vapour pressurc remains unchanged (d) Somc morc of the liquid benzene in flask A would cvaporatc. 14.
The total vapour pressure of an ideal-dilute liquid mixture of acetone and chloroform with a mole fraction of acetone of 0.0500 is 45.08 kPa at 308 K. (a) Use Raou lt's law to determine the partial vapour pressure of acetone for the mixture, given that the vapour pressure of pure acetone is 46.26 kPa at 308 K. (b) Hence calculate the partial vapour pressure of chloroform for the mixture . (c) Determine the Henry's law constant of chloroform at this temperature.(d) The Henry's law constant is lower than the vapour pressureof pure chloroform at 308 K. What does this imply about the nature of the interactions between acetone and chloroform in the liquid mixture?
3. (a) At 10 °C, the vapour pressures of pure chloroform (CHCI3) and pure dichloromethane (CH2C12) are 101 mmHg and 235 mmHg, respectively. Assume that a solution made by mixing CHCI3 and CH2C12 is ideal. i. If the vapour pressure of the resulting solution is 140 mmHg and it contains 1.25 moles of components, what is the mass of CHCI3 present in that solution.
Phenol and water form non-ideal liquid mixtures. When 7.32 g of phenol and 7.95 g of water are mixed together at 60 °C they form two immiscible liquid phases with mole fractions of phenol of 0. 0 42 and 0 .161 . (a) Calculate the overall mole fraction of phenol in the mixture. (b) Use the lever rule to determine the relative amounts of the two phases .
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What proportions of hexane and heptane should be mixed (i) by mole fraction, (ii) by mass in order to achieve the greatest entropy of mixing?
An ideal-dilute solution of chloroform and ethanol with a mole fraction of ethanol in the liquid phase Xeth = 0.9900 has a total vapour pressure of p = 17795 Torr. The vapour pressure of pure ethanol at this temperature is p*eth = 172.76Torr. (a) Use Raoult's law to calculate the partial pressure of ethanol in the vapour phase. (b) Hence determine the partial pressure of chloroform in the vapour phase . (c) Also calculate the mole fractions of chloroform and ethanol in the vapour phase. (d) Calculate the Henry's law constant for chloroform, Kchl at this temperature.
Figure 5.2 shows the experimentally determined phase diagrams for the nearly ideal solution of hexane and heptane. (a) Indicate which phases are present in each region of the diagram. (b) For a solution containing 1 mol each of hexane and heptane molecules, estimate the vapour pressure at 70 °C when vaporization on reduction of the external pressure just begins. (c) What is the vapour pressure of the solution at 70 °C when just one drop of liquid remains? (d) Estimate from the figures the mole fraction of hexane in the liquid and vapour phases for the conditions of part b. (e) What are the mole fractions for the conditions of part c? (f) At 85 °C and 760 Torr, what are the amounts of substance in the liquid and vapour phases when zheptane = 0.40?